Changing the chemical and physical properties of high valent heterobimetallic bis-(μ-oxido) Cu–Ni complexes by ligand effects

Abstract

Two new heterobimetallic [LNiO₂Cu(RPY2)]⁺ (RPY2 = N-substituted bis 2-pyridyl(ethylamine) ligands with R = indane, 3a or R = Me, 3b) complexes have been spectroscopically trapped at low temperatures. They were prepared by reacting the mononuclear side-on LNi^II superoxo precursor bearing a β-diketiminate ligand (L = [HC-(CMeNC₆H₃(iPr)₂)₂]) with the Cu(I) complexes. In contrast to the oxo groups in known high-valent [M₂(μ-O)₂]ⁿ⁺ (M = Fe, Co, Ni, Cu) cores that display electrophilic reactivities, 3a and 3b display rather nucleophilic oxo cores active in aldehyde deformylation reactions. However, the spectroscopic and reactivity properties of 3a/3b are found to be distinct relative to that of the previously reported [LNiO₂Cu(MeAN)]⁺ complex containing a more basic (nucleophilic) N,N,N′,N′,N′-pentamethyl-dipropylenetriamine (MeAN) ligand at the copper centre. The geometry and electronic properties of the copper ligands affect the electron density of the oxygen atoms of the heterodinuclear {Ni(μ-O)₂} core and 3a/3b undergo slower nucleophilic and faster electrophilic reactions than the previously reported [LNiO₂Cu(MeAN)]⁺ intermediate. The present study therefore demonstrates the tuning of the electrophilicity/nucleophilicity of the oxygen atoms of the heterobimetallic [Ni(μ-O)₂Cu]²⁺ cores by controlling the electron donation from the ancillary ligands, and underlines the significance of subtle electronic changes in the physical and chemical properties of the biologically relevant heterobimetallic metal–dioxygen intermediates.

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Introduction

The synthesis and characterisation of metal–oxygen intermediates are very important for understanding the mechanisms of transition metal mediated dioxygen activation reactions taking place in chemical and biological systems. In this context homobimetallic bis(μ-oxido) complexes with [M₂(μ-O)₂]ⁿ⁺ cores have attracted much attention and they have been extensively studied for systems involving Cu,¹ Mn,² Ni,³ Co,⁴ Fe,⁵ and Pt centres.⁶ In particular, homobimetallic copper dioxygen cores have been the subject of extensive investigations due to their possible involvement in biological oxidation reactions as key intermediates in phenol hydroxylation by tyrosinase,⁷ as well as in methane oxidation by particulate methane monooxygenase.⁸

In contrast to the homobimetallic systems, the properties of mixed-metal dioxygen species have been less explored. These types of intermediates are probably involved in various catalytic processes in metalloenzymes; for example, in cytochrome c oxidase, where a Cu^I ion cooperates with an Fe^II(heme) to activate dioxygen or in Cu–Zn superoxide dismutase, in which the superoxido ligand disproportionation is mediated through a mixed Cu–Zn metal site. The generation and the study of such mixed metal species are therefore of significant interest due to the unique properties obtained by the combination of two different metal ions. The synthesis of heterodinuclear complexes, however, presents a special challenge because of the possibility of disproportionation and selectivity problems resulting in the formation of mixtures of homo- and heterodinuclear complexes, as well as metal-site isomers. In order to overcome these problems two main strategies were previously used in the literature (Fig. 1).⁹

Fig. 1 Two main strategies for the development of heterobimetallic metal–dioxygen complexes.

The first one involves the synthesis of ligands providing different coordination environments that are specific for each of the two metal ions. An alternative route is the reaction of a well-defined dioxygen metal subunit L_nM-O₂ with a low-valent metal complex fragment L′_mM′. This last strategy has been successfully used to generate heterobimetallic oxygen-containing species with PdMo,¹⁰ CuNi,¹¹ CuGe,¹² PtCu¹³ and CuPd¹³ combinations, starting from well-defined metal–dioxygen precursors. Our contribution in the field involves the synthesis of a novel family of NiO₂M complexes generated by using a mononuclear side-on LNi^II superoxo precursor bearing a β-diketiminate (Nacnac) ligand (L = [HC-(CMeNC₆H₃(iPr)₂)₂]) system.¹⁴ Notably, this precursor is remarkably stable and can be handled at room temperature, which made it a suitable precursor for the synthesis of heterobimetallic metal–dioxygen complexes. Interestingly, in our previous studies, the electronic structure of the [NiO₂M]ⁿ⁺ core in such complexes was found to be dependent on the nature of the second metal ion, M; whereas a peroxido species¹⁵ [Ni(μ-O₂)K]ⁿ⁺ was stabilized in the presence of potassium, replacement of the monovalent potassium ion by LZn^+ 15 (L = Nacnac) or LFe^+ 16 ions initiated peroxido O–O bond scission and subsequent H-atom abstraction to generate the heterobimetallic bis(μ-hydroxo) Ni–Zn or alkoxo hydroxido Ni–Fe species, respectively. Although the fleeting [LNiO₂ML] (M = Fe, Zn) could not be isolated, in a subsequent study a related [LNiO₂Cu(MeAN)]⁺ species was stabilized at low temperature by reacting the [LNi^IIO₂] precursor with a copper triamine [Cu(MeAN)]⁺ reductant (Scheme 1A). Interestingly, the presence of Cu in the second metal binding site was shown to result in nucleophilic oxo groups in the high-valent bis-μ-oxido Ni–Cu species, and it was able to react towards aldehyde substrates, in contrast to the reported electrophilic properties of the homobimetallic NiO₂Ni, CuO₂Cu and heterobimetallic NiO₂Fe counterparts.¹⁷ In the present manuscript we now try to systematically explore how the nature of the ancillary ligand can modulate the formation, structure, electronic properties and reactivity of such high-valent heterobimetallic dioxygen species. For this purpose, we report on the synthesis, spectroscopy, DFT derived description, and reactivity studies of two new bis-μ-oxido CuNi intermediates, where the triamine MeAN ligand at Cu is replaced by relatively weaker bases/nucleophiles in the bis 2-pyridyl(ethylamine) (RPY₂; R = methyl or indane) ligand systems. Notably, the RPY₂-type ligands have been previously utilised in the formation of binuclear Cu^II₂-peroxido complexes, which were shown to exist in equilibrium with the isomeric Cu^III₂(μ-oxido) species depending on the reaction conditions.^1a The side-on peroxido dicopper(II) intermediates exhibited electrophilic character towards C–H bond oxygenation of substrates.^1f,h,i For example, on using an “indane” substrate covalently attached to the ligand (IndanePY₂, Scheme 1), intramolecular oxygen atom transfer was shown to take place in a highly regio- and stereo-selective manner leading to the cis-hydroxylated diastereoisomers of the ligand.¹⁸ The successful generation of the [LNiO₂Cu(RPY₂)]⁺ complexes now offers the opportunity to compare and contrast the reactivity of the present complexes with that of the previously reported heterodinuclear [LNiO₂Cu(MeAN)]⁺ and homodinuclear [{Cu(RPY₂)}₂O₂]²⁺ complexes.

Scheme 1 A: Generation of the [LNi^IIIO₂Cu^III(MeAN)]⁺ complex which is already reported.¹⁷ B: Generation of [LNi^IIIO₂Cu^III(RPY₂)]⁺ species 3a (3b) upon mixing a solution of the LNi^II superoxo complex 2 with the (RPY₂)Cu^I complexes 1a (or 1b).

Results and discussion

Synthesis and UV-Vis spectroscopy

The complexes 1a and 1b were prepared by mixing one molar eq. of Cu^I(CH₃CN)₄(OTf) with one molar eq. of ligand in dichloromethane. Equimolar amounts of 1a {(IndanePY₂)Cu^I(OTf)} or 1b {(CH₃PY₂)Cu^I(OTf)} and 2 were then mixed at −90 °C in dry dichloromethane leading to the immediate formation of the brownish intermediates 3a {[IndanePY₂]Cu(O₂) Ni[C-(CMeNC₆H₃(iPr)₂)₂](OTf)} and 3b {[CH₃PY₂]Cu(O₂)Ni[C-(CMeNC₆H₃(iPr)₂)₂](OTf)}, respectively (Scheme 1B). The generation of these species was monitored by UV-Vis spectroscopy following the appearance of a characteristic absorption band centred at 885 nm for 3a and 870 nm for 3b (Fig. 2). The intermediates are stable at −90 °C, but they are thermally sensitive, as indicated by bleaching of their UV-Vis absorption features upon warming to higher temperatures (see the ESI†) with t_1/2 = 2000 s at −60 °C.

Fig. 2 Absorption spectra of the Cu^I complex (solid trace) 1a, Ni^II superoxo complex 2 (dotted trace) and the 0.15 mM [Ni^III(μ-O₂)Cu^III]⁺ species 3a (dashed trace) in dichloromethane at −90 °C. Inset: X-band EPR spectrum of 3a in dichloromethane at 77 K.

EPR spectroscopy

The EPR spectra were recorded in frozen CH₂Cl₂ solutions (77 K) for 3a and 3b and are very similar for both complexes. The EPR spectrum obtained in the case of 3a is presented in Fig. 2. The spectra are composed of typical S = 1/2 rhombic signals with g₁ = 2.39, g₂ = 2.13, and g₃ = 2.005 for 3a and g₁ = 2.39, g₂ = 2.13, and g₃ = 2.006 for 3b. These EPR signals are very similar to the one reported previously for the [LNiO₂Cu(MeAN)]⁺ complex.¹⁷ Notably, no interaction of the electron spin with the nuclear spin of copper is observed for both 3a/3b, consistent with their Ni^III(μ-O)₂Cu^III assignment, in agreement with the data previously reported in the literature for the Cu–Ni analog.¹⁷

Resonance Raman spectroscopy

The resonance Raman (rRaman) spectra of 3a and 3b were recorded using 413 nm laser excitation. rRaman bands are detected at 605 cm⁻¹ and 612 cm⁻¹ for 3a and 3b, respectively (Fig. 3, ESI†), which are sensitive to ¹⁸O substitution (performed by using Ni¹⁸O₂ as a starting reagent) and downshift (Δ¹⁸O) by 31 cm⁻¹ and 29 cm⁻¹, respectively. Notably, these bands are shifted to lower energies relative to the tetra-atomic vibrational mode of the [LNi(μ-O₂)Cu(MeAN)]⁺ complex observed at 625 cm⁻¹.¹⁷ Furthermore, as previously observed, the absence of any isotope sensitive bands in the 700–1200 cm⁻¹ region excludes the possibility of the presence of peroxo or superoxo units in 3a or 3b. Interestingly, a second ¹⁸O sensitive band is also detected at 556 cm⁻¹ (Δ¹⁸O = −21 cm⁻¹) and 579 cm⁻¹ (Δ¹⁸O = −19 cm⁻¹) for 3a and 3b respectively, which was not observed in the previously reported spectrum of the [LNiO₂Cu(MeAN)]⁺ complex.

Fig. 3 Raman shifts obtained using a 413 excitation laser for 3a involving ¹⁶O (top) and ¹⁸O (bottom) atoms. Bands originated from the solvent are marked by asterisks.

DFT calculations

DFT calculations were performed on 3a and 3b in an effort to understand their structural and electronic properties as well as the origin of the additional ¹⁸O sensitive band in the rRaman spectra. DFT-optimised structures revealed a four-coordinate distorted square-planar geometry around the nickel centre. Two conformations around the copper ion were computed for each system (conformers A and B). In all cases, the copper site is in a five-coordinate square pyramidal geometry but with either the amine group (conformer A) or one pyridine group (conformer B) weakly bonded to the metal ion in the axial position. Energetic analysis conducted on both 3a and 3b showed that the minimum free energy is obtained for the conformers (A) which make these structures the most favoured one (see Table S3; ESI†). The computed structures for 3a and 3b (conformers A and B) are presented in Fig. 4, S11 and S12.†

Fig. 4 Optimised molecular structures for 3a; conformers A (top) and B (bottom).

Both spin density plots and Singly Occupied Molecular Orbitals (SOMO) reveal that 3a and 3b bear one unpaired electron located at the nickel centre (see Fig. S13 and S14; ESI†). These results confirm the presence of one low-spin Ni^III centre (S = 1/2, 3d⁷) and one low-spin Cu^III (S = 0, 3d⁸) centre in both 3a and 3b. This assignment is further confirmed by the computed EPR parameters, which are in fair agreement with the experimental data (see Table S4; ESI†). Frequency calculations were conducted on the DFT-optimised structures of the two species and Raman spectra were calculated. Vibration modes involving the oxygen ligands were predicted at 596 cm⁻¹ and 621 cm⁻¹ for 3a and 3b (Fig. S15 and S16; Table S5†), respectively, in agreement with the assignment previously proposed for the MeAN-based Cu–Ni analog.¹⁷ A second mode was calculated to be at 553 cm⁻¹ and 528 cm⁻¹ for 3a and 3b, respectively, originating from the coupling of the Ni(μ-O₂)Cu core and the Ni-coordinated β-diketiminate ligand coordinates (see Fig. S17 and S18; ESI†). Both sets of the calculated results are in good agreement with the observed rRaman bands for each complex (Table S5; ESI†). The five-coordination geometry at the Cu ions obtained in the case of RPY₂-type ligands is affecting the coordination sphere of the Ni ion in 3a and 3b and the geometry around the Ni ion appears to be significantly distorted from planarity (dihedral angle of 11.2 and 16.2°, respectively) while it is perfectly planar in the MeAN-based complex (dihedral angle of 2.3°). This explains the appearance of a new vibration in the rR spectra of 3a/3b. The spectroscopic data thus support the DFT-calculated structure and validate the formation of both 3a and 3b.

Reactivity studies

The reactivity of the complexes 3a and 3b has been investigated in a number of nucleophilic and electrophilic reactions. The nucleophilicity of 3a and 3b has been studied in reactions with benzaldehyde, and cyclohexane carboxaldehyde (CCA). The ability of 3a (3b) to undergo electrophilic Hydrogen Atom Transfer (HAT) reactions was also evaluated in reactions with 9,10-dihydroanthracene (DHA) and 1,3-cyclohexadiene (CHD) for C–H bonds and with 2,4-di-tert-butylphenol (2,4-DTBP) and 2,6-di-tert-butylphenol (2,6-DTBP) for O–H bonds. In a typical reaction preformed 3a and 3b at −60 °C were treated with an excess of the above-mentioned substrates under a pseudo first-order condition.

The disappearance of the characteristic band at 885 nm in the UV-Vis absorption spectrum was then monitored over time (Fig. 5 for reaction of 3a with CCA). Rate constants in CH₂Cl₂ at −60 °C or at −90 °C were obtained from the pseudo-first order fit of the time trace of the decay of the 885 nm band (Fig. 5). Second-order rate constants were then determined from the dependence of the first-order rate constants on the substrate concentration (Fig. 6). Second-order rate constants derived from those studies are listed in Table 1 and compared with that of the results obtained for the previously reported [LNiO₂Cu(MeAN)]⁺ intermediate. Notably, complex 3b reacts with CCA and benzaldehyde at rates significantly slower than [LNiO₂Cu(MeAN)]⁺.

Fig. 5 Spectral changes of 3a in the presence of 50 mM CCA at −60 °C. Inset: Time trace of the decay at 885 nm band upon addition of the substrate (black trace) and the first-order fit (inset: red trace).

Fig. 6 Pseudo first-order rate constants as a function of substrate concentration; the reaction of 3a with cyclohexane carboxaldehyde (left) and 2,4 di-tert-butylphenol (right) in CH₂Cl₂.

Table 1 Second order rate constants determined for different substrates by kinetic studies by UV-Vis spectroscopy

Substrates	Benzaldehyde (−60 °C)	CCA (−60 °C)	DHA (−60 °C)	CHD (−60 °C)	2,4 DTBP (−90 °C)	2,6 DTBP (−60 °C)
3a k 2/M^−1 s^−1	0.021	0.088	0.015	0.053	4.60	0.0065
3b k 2/M^−1 s^−1	0.0178	0.557	0.015	0.014	Too fast	0.0985
LNi^III[(μ-oxo)Cu^III(MeAN)]^+k2/M^−1 s^−1	0.11 (−50 °C)	Too fast (−90 °C)	Too slow (−70 °C)	0.0005 (−70 °C)	2.44 (−90 °C)	0.0001 (−80 °C)

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In contrast, in the presence of DHA, CHD, 2,4-DTBP, or 2,6-DTBP, complex 3b is found to be a better oxidant than [LNiO₂Cu(MeAN)]⁺. These studies point to the presence of less nucleophilic oxygen atoms in 3b relative to [LNiO₂Cu(MeAN)]⁺. Notably, replacement of the methyl group of the MePy₂ ligand in 3b with a bulkier indane group in 3a did not lead to any significant change in the rate constants for the reactions with DHA and benzaldehyde. However, for reactions with bulkier substrates like 2,6-DTBP, 2,4-DTBP, or CCA, a significantly reduced rate constant is observed for 3a relative to 3b. This may be attributed to the sterically induced hindered access of the substrates in the presence of the covalently attached indane group of the IndanePY₂ ligand in 3a. Analysis of the resultant solution after reactions of 3a or 3b with various substrates showed the formation of the oxidised products in 45–70% yields (Table S1; ESI†). Interestingly, for reactions with 3a no evidence of the hydroxylation of the indane moiety was observed, which is in contrast to the previous report of the intramolecular indane hydroxylation reaction mediated by the homodinuclear copper–oxygen intermediate.¹⁸

Additional DFT calculations were performed in order to further characterise the reactivity differences. Natural population analysis was performed for 3a/3b and the results were compared with those obtained for [LNi^IIIO₂Cu^III(MeAN)]⁺ (see the ESI†). The natural negative charges found at the O atoms are smaller (by −7% to −8%) in 3a and 3b with respect to those of the corresponding atoms in [LNi^IIIO₂Cu^III(MeAN)]⁺. These data indicate that the oxido cores in 3a and 3b are less electron-rich compared to that of [LNi^IIIO₂Cu^III(MeAN)]⁺. It thus correlates with the decreased nucleophilicity presently observed.

Conclusions

Examples of heterobimetallic dioxygen intermediates are extremely rare in the literature and hence, very little is known about their reactivity. This is unfortunate, as metal dioxygen cores involving non-equivalent metal-sites have been proposed as the active species in a number of biological and chemical oxidation processes, and a detailed knowledge about their reactivity can provide vital mechanistic insights. In our continuous effort to uncover structure–reactivity relationships of unprecedented dinuclear metal–dioxygen intermediates we now investigate the role of ancillary ligands in controlling the spectroscopic and reactivity properties of a heterobimetallic [Ni(μ-O)₂Cu]⁺ core. The first (and only example before this study of such a core) has been spectroscopically identified in our groups and previously shown to possess a nucleophilic oxo group that led to the deformylation of aldehydes. We now show that the nucleophilicity of the oxo groups can be tuned by varying the electron donation of the ancillary ligand at the copper centre. Thus replacement of the MeAN ligand in the previously reported [LNi(μ-O₂)Cu(MeAN)]⁺ complex by less basic/nucleophilic RPY₂ ligands in 3a/3b led to slower nucleophilic and faster electrophilic reactions in the latter. Based on the DFT calculations, the difference in reactivity has been attributed to the presence of a five coordinate copper centre and a significant distortion of the nickel centre from planarity in 3a/3b. These result in the development of lower negative charges at the oxygen atoms of 3a/3b relative to the [LNi(μ-O₂)Cu(MeAN)]⁺ complex, where a four coordinate square planar structure has been reported to be prevalent at both the Cu and Ni centres. Furthermore, for reactions with 3a no hydroxylation of the indane moiety occurred, in contrast to the previous report of the intramolecular indane hydroxylation reaction mediated by the homodinuclear {(indane-py₂)CuO₂Cu(indane-py₂)} complex. This again emphasizes the initiation of novel reactivity properties in heterodinuclear systems relative to their homobimetallic counterparts. The present results therefore underline the significance of subtle geometric and electronic changes in the physical and chemical properties of this important class of biologically relevant metal–dioxygen intermediates.

Experimental

All chemicals used in this study except for the ligands and the complexes were commercial products of the highest available purity. Commercial starting materials were used without further purification, except for 2-vinylpyridine which was distilled prior to use. Preparation and handling of air sensitive materials were performed in a N₂ glove box OMNI-Lab 2 (VAC) with O₂ and moisture concentrations less than 2 ppm. ¹H NMR spectra were recorded on a Bruker Avance III 300 MHz NMR spectrometer. UV-Vis spectra were recorded by using an Agilent 8453 diode array spectrophotometer from 300–1100 nm with samples in a 1.0 path length quartz cuvette, connected with a cryostat from Unisoku Scientific Instruments, Japan.

Synthetic procedures

General procedure of synthesis of ligands.
CH₃PY2. The ligand has been synthesized in a slightly different way from the already reported procedure.^1g To absolute MeOH (80 mL) were added 2-vinylpyridine (11 g, 0.210 mol), 2-(2-methylaminoethyl) pyridine (4.2 g, 0.030 mol), and glacial acetic acid (1.8 g, 0.060 mol). After refluxing for 5 days under argon, MeOH was evaporated and 15% NaOH was added. The product was extracted with CH₂Cl₂ (×3) and the combined organic layers were dried over Na₂SO₄. Evaporation of CH₂Cl₂ under reduced pressure left the crude product. Flash chromatography (neutral alumina, ethylacetate/MeOH, 98 : 2) afforded the ligand as a yellow product (yield: 40%).
IndanePY₂. The ligand has been synthesized according to the already reported procedure.^18a

General procedure of the synthesis of complexes

The complexes 1a and 1b have been synthesized in situ by the dropwise addition of a solution of 1 eq. Cu^I(CH₃CN)₄OTf in anhydrous dichloromethane in a solution of 1 eq. dissolved ligand in the same solvent.

General procedure for the synthesis of [LNi^III(O₂)Cu^III(RPY2)]

The greenish solution of 2 in anhydrous CH₂Cl₂ (2.5 mL; 0.15 mM) was cooled to −90 °C. Then 1 equivalent of 1a (1b) in anhydrous CH₂Cl₂ (0.1 mL) was added to yield the deep brown intermediate 3a (3b). The generation of the deep brown species 3a (3b) was monitored by the growth of the 885 nm band in the UV/vis spectrum. ¹⁸O labelled samples for rRaman experiments were prepared using the same procedure but starting from ¹⁸O labelled Ni precursor 2.

EPR spectroscopy

EPR measurements were performed on a Bruker ESP 300 X-band EPR spectrometer equipped with a fused quartz Dewar for measurements at liquid nitrogen temperature.

Resonance Raman

rRaman spectra were recorded in CH₂Cl₂ at −92 °C (Bruker cryostat) using 413 nm excitation with a Horiba Jobin-Yvon LabRAM HR800 confocal Raman spectrometer. The concentrations of samples were from 3 mM to 8 mM.

DFT calculations

All theoretical calculations were performed with the ORCA program package.¹⁹ Full geometry optimizations were carried out for all complexes using the GGA functional BP86^20–22 in combination with the TZV/P²³ basis set for all atoms and by taking advantage of the resolution of the identity (RI) approximation in the Split-RI-J variant²⁴ with the appropriate Coulomb fitting sets.²⁵ Increased integration grids (Grid4 in ORCA convention) and tight SCF convergence criteria were used. Solvent effects were accounted within the framework of the conductor like screening model (COSMO) which is a dielectric continuum approach.²⁶ Vibrational frequency calculations were performed to ensure that each geometry optimization converged to a real minimum. IR and rRaman spectra were obtained from numerical frequency calculations performed on the optimised structures using the B3LYP^27,28 functional together with the TZV/P²³ basis set. The relative energies were obtained from single-point calculations using the same combination of functional and basis sets. They were computed from the gas-phase optimised structures as a sum of electronic energy, thermal corrections to free energy, and free energy of solvation. g-Tensors^29–32 were evaluated from additional single point calculations using the B3LYP functional. Scalar relativistic effects were included with ZORA paired using the SARC def2-TZVP(-f) basis sets^33,34 and the decontracted def2-TZVP/J Coulomb fitting basis sets for all atoms. Increased integration grids (Grid4 and GridX4 in ORCA convention) and tight SCF convergence criteria were used. Picture change effects were applied and the integration grids were increased to an integration accuracy of 11 (ORCA convention) for the metal centre. Natural charges were obtained from additional single-point calculations using the Natural Population Analysis (NPA) and the B3LYP functional together with the TZV/P basis set.³⁵ Molecular orbitals, spin density plots and vibrational normal modes were visualized with Chemcraft software.³⁶

Reactivity studies

Exogenous substrate oxidation. In a typical experiment, 0.15 mM to 0.2 mM of 3a (3b) was generated at −90 °C, as discussed previously. The reactivity studies of 3a (3b) were performed at −60 °C under an inert atmosphere, by injecting the CH₂Cl₂ solution of the substrate (varying from 1 mM to 60 mM). Spectral changes at the 885 nm band were monitored by using a UV-Vis spectrum every 1 second. The pseudo-first order oxidation rate was then extracted and compared with the self decay of 3a (3b) in the absence of the substrate. If the rate of oxidation in the presence of the substrate was higher than that in the absence of the substrate, it was concluded that 3a (3b) reacted with that substrate. The pseudo-first order fitting of the decay curves yielded the rate constants (k_obs), which follow linear dependence with the concentration of the substrate. The slope of the rate constant (k_obs) versus substrate concentration fitting plot provided the second order rate constants (k₂).

Intramolecular ligand oxidation. The brownish solution of 3a was warmed up at room temperature. The solution was treated with 35% ammonia solution and after extraction with dichloromethane (×2) the organic phases were washed with brine (×2); the organic phases were collected, dried over MgSO₄ and the solvent was removed under vacuum. The resulting solid was analysed by ¹H NMR spectroscopy and mass spectrometry which showed the absence of the hydroxylated product.

Acknowledgements

This work has been carried out in the framework of COST action CM1305 (ECOSTBio) including two STSMs (STSM-CM1305-28897 and STSM-CM1305-32182). Financial support by the French Research Agency (COMEBAC/ANR-13-BSO7-0018) as well as from the DFG (Cluster of Excellence “Unifying Concepts in Catalysis”; EXC 314-2) is gratefully acknowledged. K. R. also thanks the Heisenberg-Program of DFG for financial support.

Notes and references

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Footnote

† Electronic supplementary information (ESI) available. See DOI: 10.1039/c6dt02391f

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